List of top Chemistry Questions on Equilibrium

For the following gaseous reversible reaction:
$ 3 \, \text{A}_{(g)} + \text{B}_{(g)} \rightleftharpoons \, \text{A}_3 \text{B}_{(g)} $
($ \Delta H = -q \, \text{kJ} $), the amount of product $ \text{A}_3 \text{B}_{(g)} $ is affected by
$\underline{\hspace{3cm}}$.

Consider the following equilibrium,

CO(g) + 2H₂(g) ↔ CH₃OH(g)

0.1 mol of CO along with a catalyst is present in a 2 dm³ flask maintained at 500 K. Hydrogen is introduced into the flask until the pressure is 5 bar and 0.04 mol of CH₃OH is formed. The K_p is ____ × 10^-3 (nearest integer).

Given: R = 0.08 dm³ bar K^-1mol^-1

Assume only methanol is formed as the product and the system follows ideal gas behaviour.

The pH of a 0.01 M weak acid $\mathrm{HX}\left(\mathrm{K}_{\mathrm{a}}=4 \times 10^{-10}\right)$ is found to be 5 . Now the acid solution is diluted with excess of water so that the pH of the solution changes to 6 . The new concentration of the diluted weak acid is given as $\mathrm{x} \times 10^{-4} \mathrm{M}$. The value of x is _______ (nearest integer).

For the given reaction, choose the correct expression of $K_c$ from the following: $Fe_{(aq)}^{3+}+SCN_{(aq)}^{−}⇌(FeSCN)_{(aq)}^{2+}$

Given below are two statements:
Statement (I): Aqueous solution of ammonium carbonate is basic.
Statement (II): Acidic/basic nature of salt solution of a salt of weak acid and weak base depends on $ K_a $ and $ K_b $ value of acid and the base forming it.
In the light of the above statements, choose the most appropriate answer from the options given below:

The pH at which Mg(OH)$_2$ $[K_{sp} = 1 \times 10^{-11}]$ begins to precipitate from a solution containing 0.10 M Mg$^{2+}$ ions is $ \_\_\_\_ $.

Which of the following statements is false?

Phenol does not undergo nucleophilic substitution reaction easily due to:

Amongst the given options which of the following molecules/ion acts as a Lewis acid?

At $298\, K$, the solubility of silver chloride in water is $1434 \times 10^{-3} \,g\, L ^{-1}$. The value of $-\log K _{sp}$ for silver chloride is ____.
(Given: Mass of $Ag$ is $1079\, g\, mol ^{-1}$and mass of $Cl$ is $355 \,g \,mol ^{-1}$ )

Consider the following equation: $2 SO _2(g)+ O _2(g) \rightleftharpoons 2 SO _3(g), \Delta H =-190 \,kJ$. The number of factors which will increase the yield of $SO _3$ at equilibrium from the following is _______
A. Increasing temperature
B. Increasing pressure
C. Adding more $SO _2$
D. Adding more $O _2$ E Addition of catalyst

The dissociation constant of acetic acid is $x \times 10^{-5}$ When $25 \,mL$ of $0.2 \,M \,CH _3 COONa$ solution is mixed with $25 \,mL$ of $0.02\, M \,CH _3 COOH$ solution, the $pH$ of the resultant solution is found to be equal to 5. The value of $x$ is ___

The effect of addition of helium gas to the following reaction in equilibrium state, is : $PCl _5( g ) \rightleftharpoons PCl _3( g )+ Cl _2( g )$

For reaction : $SO _2( g )+\frac{1}{2} O _2( g )= SO _3( g )$$K _{ p }=2 \times 10^{12}$ at $27^{\circ} C$ and 1 atm pressure The $K _{ c }$ for the same reaction is ____$\times 10^{13}$ (Nearest integer)(Given $R =0.082 \,L \,atm \,K ^{-1} \,mol ^{-1}$ )

pH of 1 litre of HCL solution is 1. How much water (in litres) is added to make pH=2?

K_sp of BaSO₄ is 8 × 10^–11. If the solubility in presence of 0.1 M CaSO₄ is?

The solubility product of BaSO₄ is $1 \times 10^{-10}$ at 298 K. The solubility of BaSO₄ in 0.1 M K₂SO₄(aq) is $x \times 10^{-9}$ g L⁻¹. Calculate the value of $x$.

$20 \,mL$ of $01 \,M \,NH _4 OH$ is mixed with $40\, mL$ of $005\, M \,HCl$ The $pH$ of the mixture is nearest to: (Given: $K _{ b }\left( NH _4 OH \right)=1 \times 10^{-5}, \log 2=030$, $\log 3=048, \log 5=069, \log 7=084$, $\log 11=104$ )

4.5 moles each of hydrogen and iodine is heated in a sealed ten litre vessel. At equilibrium, 3 moles of HI were found. The equilibrium constant for H₂(g) + I₂(g) ⇋ 2HI(g) is _____________ .

The equilibrium composition for the reaction PCl₃ + Cl₂ ⇌ PCI5, at 298 K is given below.
[PCl₃]_eq = 0.2 mol L^-
[Cl₂]eq = 0.1 mol L^-1,
[PCl₅]_eq = 0.40 mol L^-1
If 0.2 mol of Cl₂ is added at the same temperature, the equilibrium concentrations of PCl5 is ___ × 10^-2 mol L^-1
Given: K_c for the reaction at 298 K is 20

3O₂ (g) ⇌ 2O₃(g) for the above reaction at 298 K, K_c is found to be 3.0 x 10^-59. If the conc. of O₂ at equilibrium is 0.040 M then concentration of O₃ in M is

The pH of the solution containing 50 mL each of 0.10 M sodium acetate and 0.01 M acetic acid is
[Given pKa of CH3COOH = 4.57]

At 600 K, 2 mol of NO are mixed with 1 mol of $O_2$.

$\begin{array}{l}2NO\left(g\right)+O_2\left(g\right)\rightleftharpoons 2NO_2\left(g\right)\end{array} $

The reaction occurring as above comes to equilibrium under a total pressure of 1 atm. Analysis of the system shows that 0.6 mol of oxygen are present at equilibrium. The equilibrium constant for the reaction is _______. (Nearest integer)

20 mL of 0.1 M NH₄OH is mixed with 40 mL of 0.05 M HCl.The pH of the mixture is nearest to:(Given: K_b(NH₄OH) = 1 × 10^–5,log 2 = 0.30,log 3 = 0.48, log 5 = 0.69, log 7 = 0.84, log 11 =1.04)

The standard entropy change for the reaction $4Fe(s) + 3O_2(g) → 2Fe_2O_3(s)$ is $–550\ J K^{–1}$ at $298\ K$. The temperature in K at which the reaction attains equilibrium is ______. (Nearest Integer)
[Given: The standard enthalpy change for the reaction is $–165\ kJmol^{–1}$].